Question

A reaction at −8.0°C evolves 854.mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1atm. Be sure your answer has the correct number of significant digits.

Answer 1

Answer:  The volume of boron trifluoride gas that is collected is 18.6 L

Explanation:

According to the ideal gas equation:

PV=nRT

P = Pressure of the gas = 1 atm

V= Volume of the gas= ?

T= Temperature of the gas in kelvin =$-8.0^0C=273+(-8.0)=265K$

R= Gas constant = $0.0821Latm/Kmol$

n=  moles of gas=  854 mmol = 0.854 mol   (1mmol=0.001mol)

$1atm\times V=0.854\times 0.0821\times 265$

$V=18.6L$

Thus volume of boron trifluoride gas that is collected is 18.6 L